Ch.17 - Acids and Bases

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Tro 6th Edition

Ch.17 - Acids and Bases

문제 8

A 0.085 M solution of a monoprotic acid has a percent ionization of 0.59%. Determine the acid ionization constant (Ka) for the acid.

문제 11

Determine the pH of each solution. a. 0.20 M KCHO₂ b. 0.20 M CH₃NH₃I c. 0.20 M KI

문제 15

A solution of 0.23 mol of the chloride salt of protonated quinine (QH+), a weak organic base, in 1.0 L of solution has a pH of 4.58. What is the Kb of quinine (Q)?

문제 31a,b,d

Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. a. HNO₃(aq) b. NH₄⁺(aq) d. HC₂H₃O₂(aq)

문제 31c

Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. c. KOH(aq)

문제 32

Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base in aqueous solution according to the Arrhenius definition. a. NaOH(aq) b. H2SO4(aq) c. HBr(aq) d. Sr(OH)2(aq)

문제 33a,c

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. a. H₂CO₃(aq) + H₂O(l) ⇌ H₃O⁺(aq) + HCO₃^–(aq) c. HNO₃(aq) + H₂O(l) → H₃O⁺(aq) + NO₃^–(aq)

문제 33b

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH^–(aq)

문제 33d

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. d. C₅H₅N(aq) + H₂O(l) ⇌ C₅H₅NH⁺(aq) + OH^–(aq)

문제 34b

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. CH₃NH₂(aq) + H₂O(l) ⇌ CH₃NH₃⁺(aq) + OH^–(aq)

문제 34c

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. c. CO₃^2–(aq) + H₂O(l) ⇌ HCO₃^–(aq) + OH^–(aq)

문제 35c

Write the formula for the conjugate acid of each base. c. HCO3–

문제 36a

Write the formula for the conjugate base of each acid. a. H2SO4

문제 36b

Write the formula for the conjugate base of each acid. b. HBr

문제 36c

Write the formula for the conjugate base of each acid. c. HI

문제 36d

Write the formula for the conjugate base of each acid. d. HCHO2

문제 37

Both H₂O and H₂PO₄^– are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.

문제 39a

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). a. HNO₃

문제 39b

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). b. HCl

문제 39c

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). c. HBr

문제 39d

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). d. H₂SO₃

문제 40a

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). a. HF

문제 40b

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). b. HCHO₂

문제 40c

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). c. H₂SO₄

문제 40d

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). d. H₂CO₃

문제 41

The three diagrams represent three different solutions of the binary acid HA. Water molecules have been omitted for clarity, and hydronium ions (H3O+) are represented by hydrogen ions (H+). Rank the acids in order of decreasing strength.

문제 43

Rank the solutions in order of decreasing [H₃O⁺]: 0.10 M HCl; 0.10 M HF; 0.10 M HClO; 0.10 M HC₆H₅O.

문제 46c

Pick the stronger base from each pair. c. NO2– or NO3–

문제 51

Calculate the pH and pOH of each solution at 25 °C. a. [H3O+] = 1.7 × 10^-8 M b. [H3O+] = 1.0 × 10^-7 M c. [H3O+] = 2.2 × 10^-6 M

문제 53a

Calculate [H₃O⁺] and [OH^–] for each solution at 25 °C. a. pH = 8.55